CHAPTER 9 Stoichiometry More Conversions!
Stoichiometry Needs a balanced equation Use the balanced eqn to predict ending and / or starting amounts Coefficients are now mole ratios
Mole Ratios Example: 2Al 2 O 3 (l) 4Al(s) + 3O 2 (g) Mole Ratios: 2 mol Al 2 O 3 4 mol Al 2 mol Al 2 O 3 3 mol O 2 4 mol Al 3 mol O 2
Mole Ratios
Mole – Mole Problem A How many moles of lithium hydroxide are required to react with 20 mol CO 2, the average amount exhaled by a person each day? CO 2 (g) + 2LiOH(s) Li 2 CO 3 (s) + H 2 O(l)
Mole – Mole Problem A 20 mol X mol CO 2 (g) + 2LiOH(s) Li 2 CO 3 (s) + H 2 O(l) How many moles of lithium hydroxide are required to react with 20 mol CO 2, the average amount exhaled by a person each day? Step 1: Start with what you know from the problem.
Mole – Mole Problem A 20 mol X mol CO 2 (g) + 2LiOH(s) Li 2 CO 3 (s) + H 2 O(l) 1 mol 2 mol How many moles of lithium hydroxide are required to react with 20 mol CO 2, the average amount exhaled by a person each day? Step 2: Determine what you know from the balanced equation.
Mole – Mole Problem A CO 2 (g) + 2LiOH(s) Li 2 CO 3 (s) + H 2 O(l) How many moles of lithium hydroxide are required to react with 20 mol CO 2, the average amount exhaled by a person each day? Step 3: Set-up so units cancel & solve. 20 mol CO 2 = X mol LiOH 1 mol CO 2 2 mol LiOH
Mole – Mole Problem A CO 2 (g) + 2LiOH(s) Li 2 CO 3 (s) + H 2 O(l) How many moles of lithium hydroxide are required to react with 20 mol CO 2, the average amount exhaled by a person each day? X = 40 mol LiOH
Mole – Mole Problem B 5.3 molX mol CO 2 (g) + 2LiOH(s) Li 2 CO 3 (s) + H 2 O(l) How many moles of lithium carbonate are produced when 5.3 mol CO 2 are reacted? Step 1: Start with what you know from the problem.
Mole – Mole Problem B 5.3 molX mol CO 2 (g) + 2LiOH(s) Li 2 CO 3 (s) + H 2 O(l)1 mol How many moles of lithium carbonate are produced when 5.3 mol CO 2 are reacted? Step 2: Determine what you know from the balanced eqn.
Mole – Mole Problem B 5.3 molX mol CO 2 (g) + 2LiOH(s) Li 2 CO 3 (s) + H 2 O(l) 1 mol How many moles of lithium carbonate are produced when 5.3 mol CO 2 are reacted? Step 3: Set-up units to cancel out & solve. 5.3 mol CO 2 = X mol Li 2 CO 3 1 mol CO 2 1 mol Li 2 CO 3
Mole – Mole Problem B CO 2 (g) + 2LiOH(s) Li 2 CO 3 (s) + H 2 O(l) How many moles of lithium carbonate are produced when 5.3 mol CO 2 are reacted? X = 5.3 mol Li 2 CO 3
Mole – Mass Problems mol – g
mol – Mass Problems
1.Start with what you know. 2.Write a ratio of what you know from the problem above the equation. 3.Write a ratio of what you know from the balanced equation below. 4.Set the ratios together and Solve.
Balanced Equation: 6CO 2 (g) + 6H 2 O(l) C 6 H 12 O 6 (s) + 6O 2 (g) What is the mass of glucose (C 6 H 12 O 6 ) produced from 3.00 mol of water (H 2 O)? mol – Mass Problem C
Balanced Equation: 3.00 mol X grams 6CO 2 (g) + 6H 2 O(l) C 6 H 12 O 6 (s) + 6O 2 (g) What is the mass of glucose (C 6 H 12 O 6 ) produced from 3.00 mol of water (H 2 O)? mol – Mass Problem C Step 1: Start with what you know from the problem mol H 2 O = X g C 6 H 12 O 6
Balanced Equation: 3.00 mol X grams 6CO 2 (g) + 6H 2 O(l) C 6 H 12 O 6 (s) + 6O 2 (g) 6 mol g What is the mass of glucose (C 6 H 12 O 6 ) produced from 3.00 mol of water (H 2 O)? mol – Mass Problem C Step 2: Use the balanced equation to find the mol of known and the grams of unknown. 6 mol H 2 O = g C 6 H 12 O 6
Balanced Equation: 3.00 mol X grams 6CO 2 (g) + 6H 2 O(l) C 6 H 12 O 6 (s) + 6O 2 (g) 6 mol g What is the mass of glucose (C 6 H 12 O 6 ) produced from 3.00 mol of water (H 2 O)? mol – Mass Problem C Step 3: Set-up and solve mol H 2 O = X g C 6 H 12 O 6 6 mol H 2 O g C 6 H 12 O 6
Balanced Equation: 6CO 2 (g) + 6H 2 O(l) C 6 H 12 O 6 (s) + 6O 2 (g) What is the mass of glucose (C 6 H 12 O 6 ) produced from 3.00 mol of water (H 2 O)? mol – Mass Problem C 6 X = (3.00)(180.18) 6
Balanced Equation: 6CO 2 (g) + 6H 2 O(l) C 6 H 12 O 6 (s) + 6O 2 (g) What is the mass of glucose (C 6 H 12 O 6 ) produced from 3.00 mol of water (H 2 O)? mol – Mass Problem C X = (3.00)(180.18) 6 X = g C 6 H 12 O 6
Balanced Equation: 6CO 2 (g) + 6H 2 O(l) C 6 H 12 O 6 (s) + 6O 2 (g) What is the mass of oxygen (O 2 ) produced from 2.50 mol of water (H 2 O)? mol – Mass Problem D
Balanced Equation: 2.50 mol X grams 6CO 2 (g) + 6H 2 O(l) C 6 H 12 O 6 (s) + 6O 2 (g) What is the mass of oxygen (O 2 ) produced from 2.50 mol of water (H 2 O)? mol – Mass Problem D Step 1: Start with what you know from the problem mol H 2 O = X g O 2
Balanced Equation: 2.50 mol X grams 6CO 2 (g) + 6H 2 O(l) C 6 H 12 O 6 (s) + 6O 2 (g) 6 mol (6 * 32 = 192) What is the mass of oxygen (O 2 ) produced from 2.50 mol of water (H 2 O)? mol – Mass Problem D Step 2: Determine what you know from the balanced equation. 6 mol H 2 O = g O 2
Balanced Equation: 2.50 mol X grams 6CO 2 (g) + 6H 2 O(l) C 6 H 12 O 6 (s) + 6O 2 (g) 6 mol (6 * 32 = 192) What is the mass of oxygen (O 2 ) produced from 2.50 mol of water (H 2 O)? mol – Mass Problem D Step 3: Set-up and solve mol H 2 O = X g O 2 6 mol H 2 O g O 2
Balanced Equation: 6CO 2 (g) + 6H 2 O(l) C 6 H 12 O 6 (s) + 6O 2 (g) What is the mass of oxygen (O 2 ) produced from 2.50 mol of water (H 2 O)? mol – Mass Problem D 6 X = (2.50)(192.00) 6
Balanced Equation: 6CO 2 (g) + 6H 2 O(l) C 6 H 12 O 6 (s) + 6O 2 (g) What is the mass of oxygen (O 2 ) produced from 2.50 mol of water (H 2 O)? mol – Mass Problem D X = 80.0 g O 2
Mass – mol Problems g - mol
Mass – mol Problems
1.Start with what you know. 2.Write a ratio of what you know from the problem above the equation. 3.Write a ratio of what you know from the balanced equation below. 4.Set the ratios together and Solve.
Balanced Equation: 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O(g) How many moles of NO are formed from 824 g of NH 3 ? Mass – mol Problem E
Balanced Equation: 824 g X mol 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O(g) How many moles of NO are formed from 824 g of NH 3 ? Mass – mol Problem E Step 1: Start with what you know from the problem. 824 g NH 3 = X mol
Balanced Equation: 824 g X mol 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O(g) (4*17.01 = 68.04) 4 mol How many moles of NO are formed from 824 g of NH 3 ? Mass – mol Problem E Step 2: Determine what you know from the balanced equation g NH 3 = 4 mol NO
Balanced Equation: 824 g X mol 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O(g) (4*17.01 = 68.04) 4 mol How many moles of NO are formed from 824 g of NH 3 ? Mass – mol Problem E Step 3: Set-up your ratio. 824 g NH 3 = X mol NO g NH 3 4 mol NO
Balanced Equation: 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O(g) How many moles of NO are formed from 824 g of NH 3 ? Mass – mol Problem E 824 g NH 3 = X mol NO g NH 3 4 mol NO X = (4)(824)
Balanced Equation: 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O(g) How many moles of NO are formed from 824 g of NH 3 ? Mass – mol Problem E X = 48.4 g NO
Balanced Equation: 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O(g) How many moles of H 2 O are formed from 412 g of NH 3 ? Mass – mol Problem F
Balanced Equation: 412 g X mol 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O(g) How many moles of H 2 O are formed from 412 g of NH 3 ? Mass – mol Problem F Step 1: Start with what you know from the problem. 412 g NH 3 = X mol H 2 O
Balanced Equation: 412 g X mol 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O(g) (4*17.03 = 68.12) 6 mol How many moles of H 2 O are formed from 412 g of NH 3 ? Mass – mol Problem F Step 2: Determine what is known from the balanced equation g NH 3 = 6 mol H 2 O
Balanced Equation: 412 g X mol 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O(g) (4*17.03 = 68.12) 6 mol How many moles of H 2 O are formed from 412 g of NH 3 ? Mass – mol Problem F Step 3: Set the ratios together and Solve. 412 g NH 3 = X mol H 2 O g NH 3 6 mol H 2 O
Balanced Equation: 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O(g) How many moles of H 2 O are formed from 412 g of NH 3 ? Mass – mol Problem F X = (412)(6)
Balanced Equation: 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O(g) How many moles of H 2 O are formed from 412 g of NH 3 ? Mass – mol Problem F X = 36.3 mol H 2 O
Mass – Mass Problems g - g
Gram – Gram Problems
1.Start with what you know. 2.Write a ratio of what you know from the problem above the equation. 3.Write a ratio of what you know from the balanced equation below. 4.Set the ratios together and Solve.
Gram – Gram Problems
Gram – Gram Problem G Sn(s) + 2HF(g) SnF 2 (s) + H 2 (g) How many grams of SnF 2 are produced from the reaction of g HF?
Gram – Gram Problem G g X g Sn(s) + 2HF(g) SnF 2 (s) + H 2 (g) How many grams of SnF 2 are produced from the reaction of g HF? Step 1: Start with what you know from the problem g HF = X g SnF 2
Gram – Gram Problem G g X g Sn(s) + 2HF(g) SnF 2 (s) + H 2 (g) (2*20.01=40.02) How many grams of SnF 2 are produced from the reaction of g HF? Step 2: Determine what you know from the balanced equation g HF = g SnF 2
Gram – Gram Problem G g X g Sn(s) + 2HF(g) SnF 2 (s) + H 2 (g) (2*20.01=40.02) How many grams of SnF 2 are produced from the reaction of g HF? Step 3: Put the ratios together and Solve g HF = X g SnF g HF g SnF 2
Gram – Gram Problem G Sn(s) + 2HF(g) SnF 2 (s) + H 2 (g) How many grams of SnF 2 are produced from the reaction of g HF? X = (30.00)(156.69)
Gram – Gram Problem G Sn(s) + 2HF(g) SnF 2 (s) + H 2 (g) How many grams of SnF 2 are produced from the reaction of g HF? X = g SnF 2
Gram – Gram Problem H Sn(s) + 2HF(g) SnF 2 (s) + H 2 (g) How many grams of HF are produced from the reaction of g H 2 ?
Gram – Gram Problem H X g g Sn(s) + 2HF(g) SnF 2 (s) + H 2 (g) How many grams of HF are produced from the reaction of g H 2 ? Step 1: Start with what you know from the problem g H 2 = X g HF
Gram – Gram Problem H X g g Sn(s) + 2HF(g) SnF 2 (s) + H 2 (g) (2*20.01=40.02) (2.02) How many grams of HF are produced from the reaction of g H 2 ? Step 2: Determine what you know from the balanced equation g H 2 = g HF
Gram – Gram Problem H X g g Sn(s) + 2HF(g) SnF 2 (s) + H 2 (g) (2*20.01=40.02) (2.02) How many grams of HF are produced from the reaction of g H 2 ? Step 3: Set-up the ratios and Solve g H 2 = X g HF 2.02 g H g HF
Gram – Gram Problem H Sn(s) + 2HF(g) SnF 2 (s) + H 2 (g) How many grams of HF are produced from the reaction of g H 2 ? 2.02 X = (150.5)(40.02) 2.02
Gram – Gram Problem H Sn(s) + 2HF(g) SnF 2 (s) + H 2 (g) How many grams of HF are produced from the reaction of g H 2 ? X = 2982 g HF
To Review … When solving: Known Amount & Unit Given in Problem Known Amount & Unit from Equation = Unknown Unit Given in Problem Unknown Amount & Unit from Equation
Comparing Actual and Theoretical Yield Visual Concepts Chapter 9
Percent Yield Visual Concepts Chapter 9
1.Using the mole ratio of the reactants and products in a chemical reaction, what will you most likely be able to determine? A.rate of the reaction B.energy absorbed or released by the reaction C.chemical names of the reactants and products D.mass of a product produced from a known mass of reactants
1.Using the mole ratio of the reactants and products in a chemical reaction, what will you most likely be able to determine? A.rate of the reaction B.energy absorbed or released by the reaction C.chemical names of the reactants and products D.mass of a product produced from a known mass of reactants
3.What is the mole ratio of CO 2 to C 6 H 12 O 6 in the combustion reaction: C 6 H 12 O 6 + 6O 2 6CO 2 + 6H 2 O? A.1:1 B.1:2 C.1:6 D.6:1
3.What is the mole ratio of CO 2 to C 6 H 12 O 6 in the combustion reaction: C 6 H 12 O 6 + 6O 2 6CO 2 + 6H 2 O? A.1:1 B.1:2 C.1:6 D.6:1